Elements `A` to `E` have the following electronic configuration:
`A: [He]2s^(2) 2p^(2)`, `B: [Ne]3s^(2) 3p^(2)`, `C: [Ne]3s^(2) 3p^(3)`,
`D: [Ne]3s^(2) 3p^(4)`, `E: [Ar]4s^(2)`.
Which of the above will belong to the same group in the periodic table?

The element having the electronic configuration 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(2) is :

The element having the electronic configuration 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(2) is :

Elements A, B, C, D and E have the following electronic configuration: A: 1 s^2 2 s^2 2 p^1 B: 1 s^2 2 s^2 2 p^6 3 s^2 3 p^1 C : 1 s^2 2 s^2 2 p^6 3 s^2 3 p^3 D : 1 s^2 2 s^2 2 p^6 3 s^2 3 p^5 which among these will belong to the same group in the periodic table?

Name the element with the following electronic configurations . (a) 1s^(2)2s^(2) 2p^(6) 3s^(2) 3p^(1) (b) 1s^(2) 2s^(2) 2p^(6) 3s^(2) 3p^(6) 4s^(1)

The element having the electronic configuration 1s^(2),2s^(2)2p^(6),3s^(2)3p^(1) is

Elements A,B,C,D and E gave the following electronic configuration: A 1s^2 , 2s^2 , 2p^1 B 1s^2 2s^2 2p^6 3s^2 3p^1 C 1s^2 2s^2 2p^6 3s^2 3p^3 D 1s^2 2s^2 2p^6 3s^2 3p^5 E 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 Which among these will belong to the same group in the periodic table?

Elements a,b,c and d have the following electronic configurations: a:1s^(2),2s^(2),2p^(6) b:1s^(2),2s^(2),2p^(6),3s^(2),3p^(1) c:1s^(2),2s^(2),2p^(6),3s^(2),3p^(6) d:1s^(2),2s^(2),2s^(1) Which elements among these will belong to the same group of periodic table.

What atoms are indicated by the following configuration ? [He]2s^(1) [Ne]3s^(2)3p^(3) [Ar]4s^(2)3d^(1)